For 480.0 mLmL of a buffer solution that is 0.160 M� in CH3CH2NH2CH3CH2NH2 and 9.00×10−2 M� in CH3CH2NH3ClCH3CH2NH3Cl, calculate the initial pHpH and the final pHpH after adding 1.5×10−2 molmol of HClHCl. ( Kb(CH3CH2NH2)=5.6×10−4�b(CH3CH2NH2)=5.6×10−4.)
For 480.0 mLmL of a buffer solution that is 0.160 M� in CH3CH2NH2CH3CH2NH2 and 9.00×10−2 M� in CH3CH2NH3ClCH3CH2NH3Cl, calculate the initial pHpH and the final pHpH after adding 1.5×10−2 molmol of HClHCl. ( Kb(CH3CH2NH2)=5.6×10−4�b(CH3CH2NH2)=5.6×10−4.)
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 26QAP: You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio...
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For 480.0 mLmL of a buffer solution that is 0.160 M� in CH3CH2NH2CH3CH2NH2 and 9.00×10−2 M� in CH3CH2NH3ClCH3CH2NH3Cl, calculate the initial pHpH and the final pHpH after adding 1.5×10−2 molmol of HClHCl. ( Kb(CH3CH2NH2)=5.6×10−4�b(CH3CH2NH2)=5.6×10−4.)
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